Give the type and significant of chemical reaction. Along with their suitable example.
why chemical reaction is always accompanied with bond formation.
state whether the chemical reaction is complete ly balanced.
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Answers
In a chemical reaction, a substance converts into another substance under certain given conditions in a given time. It is important to know the rate of a chemical reaction to completely understand the reaction. Which are the slowest and the fastest reactions in the world? The study of the rate of a reaction is helpful in our day to day life as well.
Equation of Rate of a Chemical Reaction
Rate of disappearance of R = Decrease in concentration of R/time taken = -Δ[R]/Δt
and, rate of appearance of P = Increase in concentration of P/time taken = + Δ[P]/Δt
Δ[R] is a negative quantity because the concentration of the reactants is decreasing while Δ[P] is a positive quantity because the concentration of the products is increasing. While performing calculations on the rate of a chemical reaction, we multiply Δ[R] by -1 to make it a positive quantity. The above equations give the average rate of a chemical reaction which is, rav.
Therefore, the average rate of a reaction depends upon the change in concentrations of the reactants or products and the time taken for that change to occur.
Here are some common reaction types:
Oxidation-Reduction or Redox Reaction. ...
Direct Combination or Synthesis Reaction. ...
Chemical Decomposition or Analysis Reaction. ...
Single Displacement or Substitution Reaction. ...
Metathesis or Double Displacement Reaction. ...
Acid-Base Reaction. ...
Combustion. ...
Isomerization.
Types of Chemical Reactions with Examples
Types of Chemical Reactions with Examples
1) Combustion/Burning Reactions:
Reaction of some combustible matters with oxidizing elements like oxygen is called combustion reactions.After these reactions oxidized products are produced. In general, these reactions are exothermic.To have combustion reaction we must have; combustible matters, oxidizing element and necessary temperature.Examine following combustion reaction samples;
Ca(s) + 1/2O2(g) → CaO(s) + Heat
2Fe(s) + 3/2O2(g) → Fe2O3(s) + Heat
If compounds including C and H elements burn with necessary O2, products are H2O and CO2.
Example:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) +Heat
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g) + Heat
2) Combination/Synthesis Reactions:
More than one matters combine and form new matter is called combination or synthesis reactions.
X + Y → XY
2H2(g) + O2 → 2H2O(l)
N2(g) + 3H2(g) → 2NH3(g)
3) Decompositions/Analysis Reactions:
These reactions are opposite of combination reactions. One compound breaks down to other compounds or elements in decomposition reactions. For example;
XY → X + Y
2H2O(l) → 2H2(g) + O2(g)
CaCO3(s) → CaO(s) + CO2(g)
4. Displacement/Replacement Reactions:
An element reacts with compound and replace with an element of that compound. For example;
Example:
Mg(s) + Cu(NO3)2(aq) → Mg(NO3)2(aq) + Cu(s)
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
If two elements or compounds replace, we call them double displacement reactions. For instance;
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Ag replace with Na and NO3 replace with Cl.
5. Acid and Base Reactions (Neutralization Reactions):
Acidic and basic matters react with and we call these reactions neutralization reactions.
Acid + Base → Salt +Water
or
Acid + Base → Salt
Example:
HCl + NaOH → NaCl + H2O
3H2SO4 + 2Al(OH)3 → Al2(SO4)3 + 6H2O
SO3 + Na2O → Na2SO4
6. Metal + Acid Reactions:
When metals react with acids, salt and hydrogen are produced.
Metal + Acid → Salt + H2(g)
Mg + 2HCl → MgCl2 + H2(g)
Some of the metals like, Pt, Au, Hg, Cu and Ag react with acids but H2 gas is not produced instead H2O is produced.
Ag + 2HNO3 → AgNO3 + NO2(g) +H2O
7. Metal + Base Reactions:
Since metals have base property, they do not react with bases. However, there are some exceptions like Zn and Al.
Example:
Al + 3KOH → K3AlO3 + 3/2H2(g)
Zn + 2NaOH → Na2ZnO2 + H2(g)
8. Exothermic and Endothermic Reactions:
Reactions releasing heat are called exothermic reactions and reactions absorbing heat are called endothermic reactions.
Example:
2H2(g) + O2(g) → 2H2O + 68 kcal Exothermic Reaction
C(s) + 1/2O2(g) → CO2(g) + 94 kcal Exothermic Reaction
2NH3(g) + 22kcal → N2(g) + 3H2(g) Endothermic Reaction
Type of chemical reaction:
Decomposition Reactions[edit] These are the same number of synthesis reactions, with the format AB → A + B. Decomposition reactions "take things apart". ...
Single Displacement Reactions ...
Double Displacement Reactions ...
Combustion ...
Organic Reactions...
Redox
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